Question
The decomposition of HI(g) is represented by the equation:
2HI(g) <-> H2(g) + I2(g)
Kc= 64 at 25°C.
If the equilibrium concentrations of H2 and I2 at 400°C are found to be [H2] = 5.4x10-4 M and [I2] = 8.8x10-3 M, what is the equilibrium concentration of HI?
2HI(g) <-> H2(g) + I2(g)
Kc= 64 at 25°C.
If the equilibrium concentrations of H2 and I2 at 400°C are found to be [H2] = 5.4x10-4 M and [I2] = 8.8x10-3 M, what is the equilibrium concentration of HI?
Answers
DrBob222
Set up an ICE chart, substitute into Kc, and solve for HI.
Post your work if you get stuck.
Post your work if you get stuck.
Adam
2.7 × 10-4